Answer:
8.37g
Explanation:
Step 1 :
The balanced equation for the reaction. This is given below:
N2 + 2O2 —> 2NO2
Step 2:
Data obtained from the question.
Volume (V) of N2 = 2L
Pressure (P) = 840mmHg
Temperature (T) = 24°C
Number of mole (n) of N2 =?
Step 3:
Conversion to appropriate unit.
For pressure:
760mmHg = 1atm
840mmHg = 840/760 = 1.11 atm
For Temperature:
T(K) = T(°C) + 273
T(°C) = 24°C
T(K) = 24°C + 273
T(K) = 297K
Step 4:
Determination of the number of mole N2.
The number of mole of N2 can be obtained by using the ideal gas equation as follow:
Volume (V) of N2 = 2L
Pressure (P) = 1.11 atm
Temperature (T) = 297K
Number of mole (n) of N2 =?
Gas constant (R) = 0.082atm.L/Kmol
PV = nRT
Divide both side by RT
n = PV / RT
n = 1.11 x 2 / 0.082 x 297
n = 0.091 mole
Therefore, the number of mole of N2 that reacted is 0.091 mole
Step 5:
Determination of the mass of NO2 produced from the reaction. This is illustrated below:
N2 + 2O2 —> 2NO2
From the balanced equation above,
1 mole of N2 produced 2 moles of NO2.
Therefore, 0.091 mole of N2 will produce = 0.091 x 2 = 0.182 mole of NO2.
Finally, we will convert 0.182 mole of NO2 to gram as shown below:
Number of mole NO2 = 0.182 mole
Molar mass of NO2 = 14 + (16x2) = 46g/mol
Mass = number of mole x molar mass
Mass of NO2 = 0.182 x 46
Mass of NO2 = 8.37g
